Stoichiometry of Reactions in Solution

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Stoichiometry of Reactions in Solution I. Introduction: Stoichiometry of reactions in solution applied stoichiometry and the idea of a limiting reactant to a reaction in solution. This experiment involved performing aqueous acid and base titrations to determine the mole ratios of four different acid base reactions. Titration is one compound added to a known amount of another compound quantitatively and reacted together to completion (the solution turn pink at the end point). The end point is also called the neutralization point, which means that all the acid has reacted completely with the base and the solution has been neutralized. (Neutral pH=7.00). II. Experimental Procedure: This experiment required the safety glasses and gloves at all the times because acids and bases were used. The buret had used the NaOH thoroughly rinsed three times because at the first titration the NaOH solution was used. About 50Ml the NaOH solution was in a clean beaker and brought it to experiment area. A funnel was used to fill the NaOH into the buret and recorded the initial volume on the buret to the correct number of significant figures. A pipette was used to take 10.00ml HCl into a clean 50mL Erlenmeyer flask. Three drops of phenolphthalein indicator was added into the HCl solution. The stopcock was opened and the NaOH solution was added into the HCl solution. The flask was swirled to mix the solutions and titrate to a faint pink end point. Recorded the final volume on the butret and used the final volume as a beginning volume to repeat the titration. At the second titration, the experiment was exactly the same as the first titration but the H2SO4 solution was used to instead of the HCl solution. The same step as the first experiment was repeated. In the third experiment, the buret had used Ba (OH) 2 thoroughly rinsed three times. 10mL of HCl

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